1. A 0.100 M solution of a weak acid has a pH of 1.96. Calculate the [H3O+] in the solution.
2. Suppose you have a 0.100 M solution of a weak acid that has a pH of 2.07. Calculate the Ka for this acid. *Report your answer to 2 significant figures.
1. A 0.100 M solution of a weak acid has a pH of 1.96. Calculate the...
A .175 M weak acid solution has a pH of 3.25. Calculate the Ka for the acid. (hint your answer should contain three significant figures and be written in scientific notation ex. 4.67E-2 )
The weak acid HIO has a Ka of 2.0×10−11. If a 1.7 M solution of the acid is prepared, what is the pH of the solution? The equilibrium expression is: HIO(aq)+H2O(l)⇋H3O+(aq)+IO−(aq) Report your answer with two significant figures.
Calculate the pH of a 0.100 M aqueous solution of the weak acid HCHO2 (Ka = 1.80E-04)
A 0.135 M weak acid solution has a pH of 3.60. Find Ka for the acid. Express your answer using two significant figures.
1. A 0.100 M solution of the weak acid HB has a pH of 3.00. What are the [H+], [B-], and Ka for this acid? 2. A solid acid is dissolved in water. Half the solution is titrated to a phenolphthalein end point with NaOH solution. The neutralized and acid solutions are then mixed and the pH of the resulting solution is found to be 4.60. Find Ka of the solid acid. 3. Assuming your buffered solution contains acetic acid,...
Calculate the pH for both a 0.100 M solution of HClO4 and a 0.100 M solution of a HClO (Ka = 2.9 × 10–8)? (Don't forget significant figures!)
A 0.10 M solution of a weak acid, “HA”, has a pH of 5.20. Calculate [H3O+]. Keep 2 sig figs in your answer.
2. The pH of a 0.100 M solution of an acid, HA, is 1.70. Calculate the K? (use ICE) Н А Р НА pH = 1.70 2.Show your work with units and correct significant figures for all questions that involve a calculation 1. Predict the expected pH ( <7, >7, =7) at the endpoint(s) of each of the three titrations. Explain your reasoning. a. Titration of a Strong Acid, HCl, with a Strong Base, NaOH Predicted pH (circle one): (a.)...
The pH of a 4.39×10-3 M solution of a weak monoprotic acid is 4.40. Calculate Ka for this monoprotic acid to three significant figures.
Find the pH and percent ionization of a 0.100 M solution of a weak monoprotic acid having the given Ka values. (a) Ka = 1.9 10-5 (b) Ka = 1.9 10-3 (c) Ka = 1.9 10-1